[cs_content][cs_section parallax=”false” separator_top_type=”none” separator_top_height=”50px” separator_top_angle_point=”50″ separator_bottom_type=”none” separator_bottom_height=”50px” separator_bottom_angle_point=”50″ style=”margin: 0px;padding: 45px 0px;”][cs_row inner_container=”true” marginless_columns=”false” style=”margin: 0px auto;padding: 0px;”][cs_column fade=”false” fade_animation=”in” fade_animation_offset=”45px” fade_duration=”750″ type=”1/1″ style=”padding: 0px;”][cs_text]Production of Materials > 4. Electrochemical Methods >
Solve problems and analyse information to calculate the potential (E°) requirement of named electrochemical processes using tables of standard potentials and half-equations[/cs_text][/cs_column][/cs_row][/cs_section][cs_section parallax=”false” separator_top_type=”none” separator_top_height=”50px” separator_top_angle_point=”50″ separator_bottom_type=”none” separator_bottom_height=”50px” separator_bottom_angle_point=”50″ style=”margin: 0px;padding: 45px 0px 0px;”][cs_row inner_container=”true” marginless_columns=”false” style=”margin: 0px auto;padding: 0px;”][cs_column fade=”false” fade_animation=”in” fade_animation_offset=”45px” fade_duration=”750″ type=”1/1″ style=”padding: 0px;”][cs_text]
- Table of standard potentials: A table that lists common reduction half-equations along with the potentials of the half-equations, known as reduction potentials, relative to the standard hydrogen electrode.
- Oxidation potentials (potentials of the reverse half-equations to those listed) are equal in magnitude but opposite in sign to reduction potentials.
- The overall potential of an electrochemical process can be calculated by adding the reduction potential to the oxidation potential:
- If the potential is positive, then the reaction is spontaneous (i.e. it is a galvanic cell).
- If the potential is negative, then the reaction requires the application of a voltage greater than or equal to the magnitude of the potential (i.e. it is an electrolytic cell).
Table of Standard Potentials:
Extract from HSC Chemistry Data Sheet. © 2010, Board of Studies NSW. [/cs_text][/cs_column][/cs_row][/cs_section][cs_section parallax=”false” separator_top_type=”none” separator_top_height=”50px” separator_top_angle_point=”50″ separator_bottom_type=”none” separator_bottom_height=”50px” separator_bottom_angle_point=”50″ class=”cs-ta-center” style=”margin: 0px;padding: 45px 0px;”][cs_row inner_container=”true” marginless_columns=”false” style=”margin: 0px auto;padding: 0px;”][cs_column fade=”false” fade_animation=”in” fade_animation_offset=”45px” fade_duration=”750″ type=”1/1″ style=”padding: 0px;”][x_image type=”none” src=”https://easychem.com.au/wp-content/uploads/2018/04/Table-of-Standard-Potentials.png” alt=”” link=”false” href=”#” title=”” target=”” info=”none” info_place=”top” info_trigger=”hover” info_content=””][x_video_embed no_container=”false” type=”16:9″][/x_video_embed][/cs_column][/cs_row][/cs_section][/cs_content]